Chapter 9: Problem 38
How many grams of Al form from 9.73 g of aluminum oxide if the yield is 91\(\% ?\) $$\mathrm{Al}_{2} \mathrm{O}_{3}+3 \mathrm{C} \rightarrow 2 \mathrm{Al}+3 \mathrm{CO}$$
Chapter 9: Problem 38
How many grams of Al form from 9.73 g of aluminum oxide if the yield is 91\(\% ?\) $$\mathrm{Al}_{2} \mathrm{O}_{3}+3 \mathrm{C} \rightarrow 2 \mathrm{Al}+3 \mathrm{CO}$$
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Get started for freeThe following reaction can be used to remove \(\mathrm{CO}_{2}\) breathed out by astronauts in a spacecraft. $$2 \mathrm{LiOH}(s)+\mathrm{CO}_{2}(g) \rightarrow \mathrm{Li}_{2} \mathrm{CO}_{3}(s)+\mathrm{H}_{2} \mathrm{O}(l)$$ \begin{equation}\begin{array}{l}{\text { a. How many grams of carbon dioxide can }} \\ {\text { be removed by } 5.5 \text { mol LiOH? }} \\ {\text { b. How many milliliters } \mathrm{H}_{2} \mathrm{O} \text { (density }=} \\\ {0.997 \mathrm{g} / \mathrm{mL} \text { ) could form from } 25.7 \mathrm{g} \text { LiOH? }} \\ {\text { c. How many molecules } \mathrm{H}_{2} \mathrm{O} \text { could be }} \\ {\text { made when } 3.28 \mathrm{g} \mathrm{CO}_{2} \text { react? }}\end{array}\end{equation}
Assume that 44.3 \(\mathrm{g} \mathrm{Na}_{2} \mathrm{O}\) are formed during the inflation of an air bag. How many liters of \(\mathrm{CO}_{2}(\) density \(=1.35 \mathrm{g} / \mathrm{L})\) are needed to completely react with the \(\mathrm{Na}_{2} \mathrm{O}\) ? $$\mathrm{Na}_{2} \mathrm{O}(s)+2 \mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightarrow 2 \mathrm{NaHCO}_{3}(s)$$
How many grams of \(\mathrm{NaNO}_{2}\) form when 256 \(\mathrm{g} \mathrm{NaNO}_{3}\) react? The yield is 91\(\% .\) $$2 \mathrm{NaNO}_{3}(s) \longrightarrow 2 \mathrm{NaNO}_{2}(s)+\mathrm{O}_{2}(g)$$
Describe the relationship between the limiting reactant and the theoretical yield.
Write the conversion factor needed to convert from g \(\mathrm{O}_{2}\) to \(\mathrm{L} \mathrm{O}_{2}\) if the density of \(\mathrm{O}_{2}\) is 1.429 \(\mathrm{g} / \mathrm{L}\) .
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